Ch 3,4,5 Review

How many grams of water are needed to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution?

• 769 g

• 36.2 g

• 100. g

• 0.157 g

• 157 g

Consider a solution made from a nonvolatile solute and a volatile solvent. Which statement is true?

• The vapor pressure of the solution is always greater than the vapor pressure of the pure solvent.

• The boiling point of the solution is always greater than the boiling point of the pure solvent.

• The freezing point of the solution is always greater than the freezing point of the pure solvent.

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂) and 85.0 g H₂O? Kf of water is 1.86°C/m.

• 17.6°C

• −176°C

• −1.50°C

• 1.50°C

• −17.6°C

What is the molar mass of toluene if 0.85 g of toluene depresses the freezing point of 100. g of benzene by 0.47°C? Kf of benzene is 5.12°C/m.

• 92.6 g/mol

• 78.0 g/mol

• 10.7 g/mol

• 81.8 g/mol

• 927 g/mol

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO₃)₂; 0.100 m ethanol; 0.090 m NaCl.

• Mg(NO₃)₂ < NaCl < ethanol

• ethanol < Mg(NO₃)₂ < NaCl

• ethanol < NaCl < Mg(NO₃)₂

• NaCl < ethanol < Mg(NO₃)₂

• Mg(NO₃)₂ < ethanol < NaCl

What mass of Na₂SO₄ is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M?

• 3.11 g

• 24.9 g

• 12.4 g

• 6.21 g

• 8.88 g

34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H₂SO₄ solution. What is the concentration of the original sulfuric acid solution?

• 0.0229 M

• 0.218 M

• 0.0523 M

• 0.209 M

• 0.105 M

Tags

NGSS.HS-PS1-7

Which of the following aqueous solutions has the lowest freezing point?

• 0.18 m KCl

• 0.15 m Na₂SO₄

• 0.12 m Ca(NO₃)₂

• pure water

• 0.20 m C₂H₆O₂ (ethylene glycol)

A small bubble rises from the bottom of a lake, where the temperature and pressure are 4°C and 3.0 atm, to the water's surface, where the temperature is 25°C and the pressure is 0.95 atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.

• 0.72 mL

• 6.2 mL

• 41.4 mL

• 22.4 mL

• 7.1 mL

The temperature of an ideal gas in a 5.00 L container originally at 1 atm pressure and 25°C is lowered to 220 K. Calculate the new pressure of the gas.

• 1.0 atm

• 1.35 atm

• 8.8 atm

• 0.738 atm

• 0.114 atm